An atom emits a photon of light with a wavelength of 566 nanometers. How much energy has the atom lost?
Answer in units of Joules.
This is a similar problem to one you asked earlier under another screen name (Nicole).
okay. but how do you figure out how much energy the atom lost ?! i got the energy of the atom to be 3.51178 x 10^-19.
now. how do i figure out how much energy the atom lost?
We must have punched different numbers but we are close. I obtained 3.517 x 10^-19 J which rounds to 3.52 x 10^-19 J. That is not the energy of the atom, that is the energy of the photon emitting 566 nm AND that is the energy lost by the atom when emitting the 566 nm photon.
To calculate how much energy an atom has lost when it emits a photon, you can use the formula:
Energy (E) = Planck's constant (h) × Speed of light (c) / Wavelength (λ)
Where:
- Planck's constant (h) is approximately equal to 6.626 × 10^(-34) Joule-seconds
- Speed of light (c) is approximately equal to 2.998 × 10^8 meters per second
- Wavelength (λ) is given as 566 nanometers, but we need to convert it to meters by dividing it by 10^9
Let's plug in the values and calculate the energy:
Wavelength (λ) = 566 nm = 566 × 10^(-9) m
Energy (E) = (6.626 × 10^(-34) J·s × 2.998 × 10^8 m/s) / (566 × 10^(-9) m)
Simplifying the equation, we get:
E = (6.626 × 2.998 × 10^(-34) × 10^8) / (566 × 10^(-9))
E = (6.626 × 2.998) / (566) × 10^(-26+8-9) Joules
E ≈ 3.51 × 10^(-19) Joules
Therefore, the atom has lost approximately 3.51 × 10^(-19) Joules of energy.